9. The reaction 2NO +O2 → 2NO2 is believed to occur by the following mechanism: 2NO ↔ N2O2 N2O2 +...
9. The reaction 2NO +O2 → 2NO2 is believed to occur by the following mechanism:
2NO ↔ N2O2
N2O2 + O2 → 2 NO2
a. Assume N2O2 to be in a steady state and derive the rate equation for the overall reaction.
b. Under what condition does the rate equation reduce to second order kinetics in NO and first order kinetics in O2 at the same time?
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9. The reaction 2NO +O2 → 2NO2 is believed to occur by the following mechanism: 2NO ↔ N2O2 N2O2 +...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
19. For the reaction 2NO + O2 + 2NO2 the following reaction mechanism have been suggested;...
19. For the reaction 2NO + O2 + 2NO2 the following reaction mechanism have been suggested; step1: NO + NO NZOZ Fast step 2: N2O2 + O2 k2, 2NO2 Slow and the apparent rate law was found to be R = kes [NO]? What would be the estimated effective activation energy, Eel, value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol- and 205 kJ mol', respectively, and the activation energy of step...
2. For reaction (E), write the expression for the steady-state concentration of N2O2, [N2O2]ss. What is...
2. For reaction (E), write the expression for the steady-state concentration of N2O2, [N2O2]ss. What is the steady-state concentration of N2O2 given a concentration of [NO] = 1 ppb and [H2] = 500 ppb? Solve for the production rate (molecules cms-1) of N20. Assume the number density of air molecules is 2.5x1019 molecules cm3. The following reaction mechanisms we have discussed to some degree during class: (A) HNO3 → OH + NO2 (ka = 0.12 s-1) (B) CO+O → CO2...
3. According to the mechanism 2NO ki ki N202 N202 + 02 -k2 → 2NO2 Under...
3. According to the mechanism 2NO ki ki N202 N202 + 02 -k2 → 2NO2 Under steady state approximation, what is the rate of formation, (v), of nitrogen dioxide, NO2, when the oxygen concentration is very low?
Question 6: Reaction Mechanisms (9 points) For the reaction: 2NO2 → 2NO + O2 Suppose there are two possible mechanisms t...
Question 6: Reaction Mechanisms (9 points) For the reaction: 2NO2 → 2NO + O2 Suppose there are two possible mechanisms to define a particular reaction. These two mechanisms are proposed below: 1. NO2 → NO + O (slow) O + NO2 → O2 + NO (fast) 2. 2NO2 → NO3 + NO (slow) NO3 → NO + O2 (fast) a) Identify the rate for each reaction and the order of each reaction. (4 points) b.) Identify the intermediate for each...
The reaction of NO with O2 to give NO2 is an important process in the formation...
The reaction of NO with O2 to give NO2 is an important process in the formation of smog in any large city: 2NO+ O2 + 2NO2 Experiments show that this reaction is third order overall. The following mechanism has been proposed: NO + NON202 N202 + O2 NO2 + NO2 (a) If the second step is rate-determining, what is the rate law? e rate law? [NO] Rate = k2 [02] (6) Is this rate law consistent with the overall third-order...
The reaction 2NO(g)+O2(g)→2NO2(g) is second order in NO and first order in O2. When [NO]= 4.5×10−2...
The reaction 2NO(g)+O2(g)→2NO2(g) is second order in NO and first order in O2. When [NO]= 4.5×10−2 M and [O2]= 3.7×10−2 M , the observed rate of disappearance of NO is 9.9×10−5 M/s . What is the rate of disappearance of O2 at this moment?
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54...
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
- For the reaction 2NO + O2 + 2NO the following reaction mechanism have been suggested;...
- For the reaction 2NO + O2 + 2NO the following reaction mechanism have been suggested; steps: NO + NON2O2 Fast step 2: N2O2 + O2 k2 2NO Slow and the apparent rate law was found to be R = kerr [NO] What would be the estimated effective activation energy, El. value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol" and 205 kJ moll, respectively, and the activation energy of step 2...
9. Consider the reaction below; (6 points) N2O2(g) + O2(g) + 2NO2(g) When the reaction is...
9. Consider the reaction below; (6 points) N2O2(g) + O2(g) + 2NO2(g) When the reaction is performed at 250.0°C and again at 325.0°C, the rate constant increases by a factor of 5.6. Use the information to calculate the activation en reaction.
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
19. For the reaction 2NO + O2 + 2NO2 the following reaction mechanism have been suggested; step1: NO + NO NZOZ Fast step 2: N2O2 + O2 k2, 2NO2 Slow and the apparent rate law was found to be R = kes [NO]? What would be the estimated effective activation energy, Eel, value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol- and 205 kJ mol', respectively, and the activation energy of step...
2. For reaction (E), write the expression for the steady-state concentration of N2O2, [N2O2]ss. What is the steady-state concentration of N2O2 given a concentration of [NO] = 1 ppb and [H2] = 500 ppb? Solve for the production rate (molecules cms-1) of N20. Assume the number density of air molecules is 2.5x1019 molecules cm3. The following reaction mechanisms we have discussed to some degree during class: (A) HNO3 → OH + NO2 (ka = 0.12 s-1) (B) CO+O → CO2...
3. According to the mechanism 2NO ki ki N202 N202 + 02 -k2 → 2NO2 Under steady state approximation, what is the rate of formation, (v), of nitrogen dioxide, NO2, when the oxygen concentration is very low?
The reaction of NO with O2 to give NO2 is an important process in the formation of smog in any large city: 2NO+ O2 + 2NO2 Experiments show that this reaction is third order overall. The following mechanism has been proposed: NO + NON202 N202 + O2 NO2 + NO2 (a) If the second step is rate-determining, what is the rate law? e rate law? [NO] Rate = k2 [02] (6) Is this rate law consistent with the overall third-order...
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
- For the reaction 2NO + O2 + 2NO the following reaction mechanism have been suggested; steps: NO + NON2O2 Fast step 2: N2O2 + O2 k2 2NO Slow and the apparent rate law was found to be R = kerr [NO] What would be the estimated effective activation energy, El. value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol" and 205 kJ moll, respectively, and the activation energy of step 2...
9. Consider the reaction below; (6 points) N2O2(g) + O2(g) + 2NO2(g) When the reaction is performed at 250.0°C and again at 325.0°C, the rate constant increases by a factor of 5.6. Use the information to calculate the activation en reaction.
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